Just finished the video and this was seriously so amazing. It clarified all of the questions I've been having and showed me how to do everything I've been stuck on. You are definitely one of the best professors I've seen. Thank you for this amazing resource
Thank you, Chad for the great lectures. At 17:53 you said to multiply concentration based on a molar ratio. Is this right for all types of salts (whether basic or acidic)? Is it the subscript of "i" in the original equation that represents the molar ratio? Thank you for your support!!
Multiplying by the mole-to-mole ratio which is just the subscript for F in the formula. Since NaF only has a single F, 0.1M NaF will result in 0.1M F- concentration. But had we had 0.1M MgF2, then the F- concentration would have been double that at 0.2M. Hope this helps!
Hi Michael. Unfortunately, I'll be releasing chapter 17 on Buffers, Titrations, and Solubility Equilibria (Ksp) next week, but it is already in my old General Chemistry playlist. Here's the first lesson in chapter 17 on buffers: th-cam.com/video/eCKirIijRZc/w-d-xo.html Hope this helps and best wishes tomorrow!
I cover Coordination Chemistry briefly in my old Gen Chem playlist: th-cam.com/video/r-D-5d1fJMc/w-d-xo.html It corresponds to chapter 21 so I won't get to the new ones until later in the spring. This won't be as thorough as what you might see in an advanced inorganic class but you should still find it useful. I have a survey course in thermodynamics (physical chemistry). It isn't on youtube but you'll find it embedded on my site free here: www.chadsprep.com/chads-elementary-physical-chemistry-videos/ You could definitely do a more robust treatment of the subject than this, but it is definitely a more thorough treatment of the subject than the thermochemistry and thermodynamics chapters in my gen chem playlists. And unfortunately group theory and quantum chemistry will have to be future projects...I envision an entire semester spent on quantum. Hope this helps!
There are actually a few exceptions to this. Note that the only one included in the lesson was HSO4-, but there are a few others that are part of polyprotic series that are amphoteric but are more acidic than basic. Other notable examples of amphoteric anions that are more acidic than basic include HC2O4-, H3P2O7-, and H2AsO4-. There is no set of rules here that doesn't have exceptions, and there is no way of knowing these except to look up their Ka values and to calculate the corresponding Kb values to see if they are more acidic or more basic...or pure memorization. So I stick with teaching the general trend and include a common exception students are likely to encounter (well knowing there are others). I've seen the conjugate base of phosphoric and oxalic show up once each, but the rest never. Hope this helps!
Thank you - my professor mentioned and talks about how she learns still from you. Just starting on this journey in healthcare - Trying to finish out ACS and Final this week- appreciate the kind help and excellence!!
Hey Chad! Thank you so much for doing these videos! They're extremely helpful. Quick question, around 8:13 you mention how size relates to acidity with elements in the same group. I always thought the trend for acidity increased moving down a group. Is this different because we are dealing with transition metals?
Hi Dakota! The trend you site is the trend for binary acids such as HF, HCl, HBr, HI. The longer the bond to hydrogen, the weaker the bond and the more likely it is to dissociate...so the stronger the acid. But when we talk about the acidity of cations, we are not talking about binary acids or of anything bonded to hydrogen at all. Rather, we are talking about the ability of cations to act as electron acceptors (Lewis acids). And the smaller the cation, the greater its charge density and the greater the 'attraction' to electrons. Hope this helps!
lmao was looking for this video... came out 3 hours ago... amazing. chad for 2024... ill vote for you
I'll stick to my day job...yikes!😜
Chad you’re an excellent lecturer. Very talented
Thank you!
I'm literally only 3mins into the video and this is already so so so helpful. Thank you! Very easy to understand and clear.
Glad it was helpful!
Just finished the video and this was seriously so amazing. It clarified all of the questions I've been having and showed me how to do everything I've been stuck on. You are definitely one of the best professors I've seen. Thank you for this amazing resource
I scored 100% in all my exams in chem 1 thanks TO YOU. Here I am in gen 2 following the same trends. I can't thank you ENOUGH.
Excellent - great job!
Thank you, Chad for the great lectures. At 17:53 you said to multiply concentration based on a molar ratio. Is this right for all types of salts (whether basic or acidic)? Is it the subscript of "i" in the original equation that represents the molar ratio?
Thank you for your support!!
Multiplying by the mole-to-mole ratio which is just the subscript for F in the formula. Since NaF only has a single F, 0.1M NaF will result in 0.1M F- concentration. But had we had 0.1M MgF2, then the F- concentration would have been double that at 0.2M. Hope this helps!
I am confused about one part. Aren't cations electron donors? Since their final charge is positive?
Noo cations have a deficiency of electrons, and something that has a deficiency of something can't have the ability to donate it.
I dont know if you know the impact of what you do for us. Your a blessing from God
Glad to hear it and Thank You very much.
Thanks for this video! If the conjugate base of a weak acid is a strong base, then why wouldn't F- be classified as a strong base?
F- would still be a weak base regardless since it only partially associates in solution
Another incredile video. You're carrying me through chemistry!
Glad the channel is helping you succeed!
BaF2 should be neutral i guess. Ba if from a strong Base and F is from a strong acid
Acid Base KSP test tomorrow!
Hi Michael. Unfortunately, I'll be releasing chapter 17 on Buffers, Titrations, and Solubility Equilibria (Ksp) next week, but it is already in my old General Chemistry playlist. Here's the first lesson in chapter 17 on buffers: th-cam.com/video/eCKirIijRZc/w-d-xo.html
Hope this helps and best wishes tomorrow!
Nice sir, need, statistical thermodynamics, group theory, coordination compounds and advanced quantum chemistry videos sir..,
I cover Coordination Chemistry briefly in my old Gen Chem playlist: th-cam.com/video/r-D-5d1fJMc/w-d-xo.html
It corresponds to chapter 21 so I won't get to the new ones until later in the spring. This won't be as thorough as what you might see in an advanced inorganic class but you should still find it useful.
I have a survey course in thermodynamics (physical chemistry). It isn't on youtube but you'll find it embedded on my site free here: www.chadsprep.com/chads-elementary-physical-chemistry-videos/
You could definitely do a more robust treatment of the subject than this, but it is definitely a more thorough treatment of the subject than the thermochemistry and thermodynamics chapters in my gen chem playlists.
And unfortunately group theory and quantum chemistry will have to be future projects...I envision an entire semester spent on quantum.
Hope this helps!
@@ChadsPrep ok ok thank you so much sir 🙏🙏🙏💕
@@RelaxRailRide You should check out Edx. MIT's chem 1 course has many quantum chem lessons. That's not the same course that they have on YT btw.
Your method does not work with KH2PO4
can you explain this a little further?
@@ChadsPrep K+ and H2PO4-
K+ is neutral, but H2PO4- is NOT Basic. It is amphoteric and behaves as Acid.
There are actually a few exceptions to this. Note that the only one included in the lesson was HSO4-, but there are a few others that are part of polyprotic series that are amphoteric but are more acidic than basic. Other notable examples of amphoteric anions that are more acidic than basic include HC2O4-, H3P2O7-, and H2AsO4-. There is no set of rules here that doesn't have exceptions, and there is no way of knowing these except to look up their Ka values and to calculate the corresponding Kb values to see if they are more acidic or more basic...or pure memorization. So I stick with teaching the general trend and include a common exception students are likely to encounter (well knowing there are others). I've seen the conjugate base of phosphoric and oxalic show up once each, but the rest never. Hope this helps!
thank you for this short cut ive been using the ICE method for so long, it works but it takes a lot of time and i kind of get confused 🥹🥹🥹
You're welcome - Happy Studying!
Thank you - my professor mentioned and talks about how she learns still from you. Just starting on this journey in healthcare - Trying to finish out ACS and Final this week- appreciate the kind help and excellence!!
Glad the channel helps you!
Excellent lecture.... really helpful
Thank you!
Hey Chad! Thank you so much for doing these videos! They're extremely helpful. Quick question, around 8:13 you mention how size relates to acidity with elements in the same group. I always thought the trend for acidity increased moving down a group. Is this different because we are dealing with transition metals?
Hi Dakota! The trend you site is the trend for binary acids such as HF, HCl, HBr, HI. The longer the bond to hydrogen, the weaker the bond and the more likely it is to dissociate...so the stronger the acid. But when we talk about the acidity of cations, we are not talking about binary acids or of anything bonded to hydrogen at all. Rather, we are talking about the ability of cations to act as electron acceptors (Lewis acids). And the smaller the cation, the greater its charge density and the greater the 'attraction' to electrons. Hope this helps!
@@ChadsPrep That definitely helps and clears things up. Thank you so much!
@@dakotasanto66 Excellent!
Incredible lesson!
Thanks!